Consider the reaction: 2CH4(g) + 3O2(g) + 2NH3(g) --> 2HCN(g) + 6H2O(g)
If 203.5 g NH3 is reacted with excess CH4 and O2, what mass in grams of HCN can be produced?
NH3 = 14 + 3 = 17 grams/mol
203.5/17 = 12 mols of NH3
so
12 mols of HCN result
HCN = 1 + 12 + 14 = 27 grams/mol
so 12 * 27 grams HCN
To determine the mass of HCN produced, we need to follow these steps:
Step 1: Write the balanced chemical equation:
2CH4(g) + 3O2(g) + 2NH3(g) → 2HCN(g) + 6H2O(g)
Step 2: Calculate the molar mass of NH3:
Molar mass of NH3 = 14.01 g/mol + (3 * 1.01 g/mol) = 17.04 g/mol
Step 3: Convert the given mass of NH3 into moles:
moles of NH3 = mass of NH3 / molar mass of NH3
moles of NH3 = 203.5 g / 17.04 g/mol = 11.94 mol
Step 4: Use the stoichiometric coefficients from the balanced equation to find the moles of HCN formed:
From the balanced equation, we can see that the stoichiometric coefficient ratio of NH3 to HCN is 2:2.
So, moles of HCN = 11.94 mol
Step 5: Calculate the mass of HCN:
mass of HCN = moles of HCN * molar mass of HCN
mass of HCN = 11.94 mol * (27.03 g/mol + 1.01 g/mol) = 352.13 g
Therefore, the mass of HCN produced is 352.13 grams.
To find the mass of HCN produced, we need to use the concept of stoichiometry, which is the study of the quantitative relationships between reactants and products in a chemical reaction.
1. Start by writing down the balanced chemical equation for the reaction:
2CH4(g) + 3O2(g) + 2NH3(g) → 2HCN(g) + 6H2O(g)
This equation shows the stoichiometric coefficients (the numbers in front of the compounds) which represent the ratio of moles of each substance involved in the reaction.
2. Convert the given mass of NH3 (203.5 g) to moles. To do this, divide the mass of NH3 by its molar mass. The molar mass of NH3 is calculated by adding up the atomic masses of each element in the compound:
Molar mass of NH3 = (1 * atomic mass of N) + (3 * atomic mass of H)
You can find the atomic masses of N and H on the periodic table.
3. Once you have the moles of NH3, you can use the stoichiometric coefficients of NH3 and HCN to determine the moles of HCN produced. According to the balanced equation, 2 moles of NH3 will produce 2 moles of HCN.
4. To convert the moles of HCN to grams, multiply the moles of HCN by its molar mass. The molar mass of HCN is calculated by adding up the atomic masses of its constituent elements:
Molar mass of HCN = (1 * atomic mass of H) + (1 * atomic mass of C) + (1 * atomic mass of N)
5. Finally, you will have the mass of HCN produced in grams.
By following these steps, you will be able to calculate the mass of HCN produced when 203.5 g of NH3 is reacted with excess CH4 and O2.